Select the correct total ionic equation for the reaction of iron(III) nitrate with sodium hydroxide.Read each answer choice carefully.Fe(NO3)з (aq) + 3NaOH (аq) — Fe(ОН)з (s) + 3NaNO3 (aq)Fe3+(aq) + 3NO3 (аq) + 3Na* (аq) + зон (аq) —> Fe(ОН)з (s) + 3Na* (aq) + 3NO3 (aq)O NO3 (aq) + Na* (aq) → NaNO3 (s)O Fe(NO3)з (аq) + 3NaOH (аq) — Fe(ОH)3 (аq) + 3NaNO3 (s)O Fe3+ (aq) + 3он (ад) — Fe(OН)з (s)O Fes* (aq) + 3NO3 (aq) + 3Na* (aq) + 3он (аq) — Fes* (aq) + 3он (аq) + 3NaNOз (s)

According to solubility rules, All nitrates are soluble. So, Fe(NO3)3 is soluble. It ionizes into…

Select the correct total ionic equation for the reaction of iron(III) nitrate with sodium hydroxide. Read each answer choice carefully. Fe(NO3)з (aq) + 3NaOH (аq) — Fe(ОН)з (s) + 3NaNO3 (аq) Fest (aq) + 3NO3° (aq) + 3Na* (aq) + 30H¯ (aq) → Fe(OH)3 (s) + 3Na* (aq) + 3NO3 (aq) + NO3 (aq) + Na* (aq) → NaNO3 (s) Fe(NO3)3 (aq) + 3NAOH (aq) → Fe(OH)3 (aq) + 3NaNO3 (s) Fe3+ (aд) + 3ОН (аq) — Fe(ОH)з (s) Fe3+ (aд) + 3NO3 (аq) + 3Na* (аq) + 3он (ад) — Fe$* (aq) + 3ОН (аq)+ 3NaNO3 (s)

Select the correct total ionic equation for the reaction of iron(III) nitrate with sodium hydroxide. Read each answer choice carefully. Fe(NO3)з (aq) + 3NaOH (аq) — Fe(ОН)з (s) + 3NaNO3 (аq) Fest (aq) + 3NO3° (aq) + 3Na* (aq) + 30H¯ (aq) → Fe(OH)3 (s) + 3Na* (aq) + 3NO3 (aq) + NO3 (aq) + Na* (aq) → NaNO3 (s) Fe(NO3)3 (aq) + 3NAOH (aq) → Fe(OH)3 (aq) + 3NaNO3 (s) Fe3+ (aд) + 3ОН (аq) — Fe(ОH)з (s) Fe3+ (aд) + 3NO3 (аq) + 3Na* (аq) + 3он (ад) — Fe$* (aq) + 3ОН (аq)+ 3NaNO3 (s)

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 46PS: Balance each of the following equations, and then write the net ionic equation. Show states for all...

See similar textbooks

Similar questions

Aqueous solutions of ammonium sulfide and mercury(II) nitrate react and a precipitate forms. (a) Write the overall balanced chemical equation and indicate the state (aq) or (s) for each compound. (b) Name each product. (c) Write the complete ionic equation. (d) Write the net ionic equation.
The formation of water-Insoluble silver chloride is useful in the analysis of chloride-containing substances. Consider the following unbalanced equation: BaCl2(aq) + AgNO3(aq) AgCI(s) + Ba(NO3)2(aq) (a) Write the balanced equation. (b) What mass of AgNO3, in grams, is required for complete reaction with 0.156 g of BaCI2? What mass of AgCI is produced?
Magnesium metal (a component of alloys used in aircraft and a reducing agent used in the production of uranium, titanium, and other active metals) is isolated from sea water by the following sequence of reactions: Mg2+(aq)+Ca(OH)2(aq)Mg(OH)2(s)+Ca2+(aq)Mg(OH)2(s)+2HCl(aq)MgCl2(s)+2H2O(l)MgCl2(l)electrolysisMg(s)+Cl2+Cl2(g) Sea water has a density of 1.026 g/cm3 and contains 1272 parts per million of magnesium a5 Mg2+(aq) by mass. What mass, in kilograms, of Ca(OH)2; is required to precipitate 99.9% of the magnesium in 1.00103 L of sea water?
On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
Gold metal will dissolve only in aqua regia, a mixture of concentrated hydrochloric acid and concentrated nitric acid in a 3:1 volume ratio. The products of the reaction between gold and the concentrated acids are AuCl4-(aq), NO(g), and H2O. The equation for this reaction where HNO3 and HCl are strong acids is Au(s)+4Cl(aq)+4H+(aq)+NO3(aq)AuCl4(aq)+NO(g)+2H2O(a) What stoichiometric ratio of hydrochloric acid to nitric acid should be used? (b) What volumes of 12 M HCl and 16 M are HNO3 required to furnish the Cl- and NO3- ions to react with 25.0 g of gold?
One of the ways to remove nitrogen monoxide gas, a serious source of air pollution, from smokestack emissions is by reaction with ammonia gas, NH3. The products of the reaction, N2 and H2O, are not toxic. Write the balanced equation for this reaction. Assign an oxidation number to each element in the reactants and products, and indicate which element is oxidized and which is reduced.
You are given a solid mixture of NaNO2 and NaCl and are asked to analyze it for the amount of NaNO2 present. To do so, you allow the mixture to react with sulfamic acid, HSO3NH2, in water according to the equation NaNO2(aq) + HSO3NH2(aq) NaHSO4(aq) + H2O() + N2(g) What is the weight percentage of NaNO2 in 1.232 g of the solid mixture if reaction with sulfa-mic acid produces 295 mL of dry N2 gas with a pressure of 713 mm Hg at 21.0 C?
In a common experiment in the general chemistry laboratory, magnesium metal is heated in air to produce MgO. MgO is a white solid, but in these experiments it often looks gray, due to small amounts of Mg3N2, a compound formed as some of the magnesium reacts with nitrogen. Write a balanced equation for each reaction.
Vitamin C, ascorbic acid (C6HgO6)(molar mass 176.1 g/mol), is a reducing agent. One way to determine the ascorbic acid content of a sample is to mix the acid with an excess of iodine, C6HgO6(aq) + I2(aq) + H2O(l) C6HgO6(aq) + 2 H3O+(aq) + 2 I(aq) and then titrate the iodine that did not react with the ascorbic acid with sodium thiosulfate. The balanced, net ionic equation for the reaction occurring in this titration is I2(aq) + 2 S2O32(aq)2 I(aq) + S4O62(aq) Suppose 50.00 mL of 0.0520 M I2 was added to the sample containing ascorbic acid. After the ascorbic acid/I2, reaction was complete, the I2 not used in this reaction required 20.30 mL of 0.196 M Na2S2O3 for titration to the equivalence point. Calculate the mass of ascorbic acid in the unknown sample.
3.93 Adipic acid is used in the production of nylon, so it is manufactured in large quantities. The most common method for the preparation of adipic acid is the reaction of cyclohexane with oxygen. Balance the skeleton equation shown be1ow.
Write an equation from the following description: reactants are gaseous NH3 and O2, products are gaseous NO2 and liquid H2O, and the stoichiometric coefficients are 4, 7, 4, and 6, respectively.
Balance the following equations: (a) for the reaction to produce "superphosphate" fertilizer Ca3(PO4)2(s) + H2SO4(aq) Ca(H2PO4)2(aq) + CaSO4(s) (b) for the reaction to produce diborane, B2H6 NaBH4(s) + H2SO4(aq) B2H6(g) + H2(g) + Na2SO4(aq) (c) for the reaction to produce tungsten metal from tungsten(VI) oxide WO3(s) + H2(g) W(s) + H2O() (d) for the decomposition of ammonium dichromate (NH4)2Cr2O7(s) N2(g) + H2O() + Cr2O3(s)